find the osmolarity for each of the following solutions, and indicate the units at the end
1) 340 μM Na2HPO4 2) 1.7 mM KH2PO4
find the osmolarity for each of the following solutions, and indicate the units at the end...
For the following solutions indicate if they are isosmotic with the intracellular fluid of a red blood cell (assume red blood cell osmolarity is 300 mOsm). Also indicate if red blood cells would swell or shrink if placed in a given solution. Solution Osmolarity (Osm) Osmolarity (hyper, iso,hypo) Tonicity (hyper, iso, or hypo) Hemolysis (Yes or No) 150 mM NaCl ddH2O 100 mM NaCl 50 mM NaCl 300 mM sucrose 150 mM CaCl2 300 mM urea 900 mM urea 900...
What is the osmolarity of each of the following solutions? 1) 3%(m/v)NaCl (strong electrolyte), used to treat hyponatremia 2) 2.5%(m/v) dextrose (C6H12O6), used to hydrate cells
7) Determine the osmolarity (called total molarity in Armstrong) of 0.10M solutions of each of the solutes listed above. Osm = nM where n is the number of moles of solute particles in solution (from above a) 0.10M NaCI= Osm b) 0.10M sucrose = Osm C) 0.10M Mg(NO3)2 = Osm d) 0.20M NaHCO3 = Osm
*1-8. Represent each of the following combinations of units in the correct SI form using an appropriate prefix: (a) Mg/mm, (b) mN/us, (c) um Mg. 1-12. Evaluate each of the following to three significant figures and express each answer in SI units using an appropriate prefix: (a) (684 μm)/(43 ms), (b) (28 ms)(0.0458 Mm)/(348 mg), (c) (2.68 mm)(426 Mg).
For each mole of H3PO4 and of Na2HPO4 mixed in aqueous solutions: a. 2 mols of H2PO4- are formed b. 1 mol of H2PO4- is formed c. No reaction occurs
Calculate the pH of each of the solutions and the change in pH to 0.01 pH units caused by adding 10.0 mL of 2.52-M HCl to 340. mL of each of the following solutions. Change is defined as final minus initial, so if the pH drops upon mixing the change is negative. + 18.55/24 points Previous Answers My Notes Calculate the pH of each of the solutions and the change in pH to 0.01 pH units caused by adding 10.0...
Calculate [H+] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. 1.[OH−]= 8.0×10−9 M . Express your answer using two significant figures. 2.A solution in which [OH−] is 100 times greater than [H+]. Express your answer using two significant figures. Can someone show every step to do this by,
For each of the following bonds, indicate the positive δ+ end and the negative δ− end. Draw an arrow to show the dipole for each. N−F <Bonding - molecular structure Problem 10.29 < 7 of 15 8+ For each of the following bonds, indicate the positive 87 end and the negative end. Draw an arrow to show the dipole for each. - Part A N - F Drag the appropriate labels to their respective targets.
11. Indicate whether each of the following aqueous solutions is acidic, basic, or neutral: KI, KF, HF.
anawer all 2 questions pleaseeeee 11. Indicate each of the following aqueous solutions is acidic, basic, or neutral: KF KI HI КОН 12. A metal complex is Cr(H2O)2Bra a) Name the complex (25 pt) Give formulas of ligands. b) What is charge of Cr? c) Find the coordination number of the complex. d) e) Sketch all possible geometric isomers, labeling cis/trans.